looking for help on the following, paticularly section 2 of this two part question 1. A...
looking for help on the following, paticularly section 2 of this two part question
1. A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 5.00 mL of 2.00 x 10-3 M KSCN. She finds
that in the equilibrium mixture the concentration of FeSCN2+ is 1.40 x 10-4 M.
a) What is the initial concentration in solution of the Fe3+ and SCN-?
b) What is the equilibrium constant for the reaction?
2. Assume that the reaction studied is actually: Fe3+ (aq) + 2 SCN- (aq) ↔ Fe(SCN)2+ (aq)
a) What is the equation for determining the equilibrium constant?
b) Using the information from question 1 and assuming [Fe(SCN)2+]eq = 1.40 x 10-4 M, calculate
the equilibrium concentration of Fe3+ and SCN-
.
c) Determine the numerical value of K.
Homework Answers
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looking for help on
the following, paticularly section 2 of this two part
question
1. A...
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL...
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x...
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C.
A student mixes 5.12 mL of 4.02 x 10...
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN.
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN. The student finds that the equilibrium concentration of FeSCN2+ is 5.6 x 10-4M. a. Set up the Kc expression for the following equation. Fe3+ + SCN- ↔ FeSCN2+b. What is the total volume of the solution? _______ mL c. Fill in the following table for the moles of each species.d. Find the concentration for the above ions. e. Calculate Kc for the reaction.
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction...
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction 1. A student mixes 5.00 mL 2.00 X 10M Fe(NO), with 5.00 ml 2.00 x 10-M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN is 1.40 x 10M. Find K for the reaction Fe(aq) + SCN (aq) FeSCN2(aq). Step 1 Find the number of moles Fe and SCN initially present. (Use Eq. 3.) (5.00 x103 LX (300X163) = (x 103...
A student mixes 5.00 mL of 2.00 times 10^-3 M Fe(NO_3)_3 with 5.00 mL of 2.00...
A student mixes 5.00 mL of 2.00 times 10^-3 M Fe(NO_3)_3 with 5.00 mL of 2.00 times 10^-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2^+ is 1.40 times 10^-4 M. a) What is the initial concentration in solution of the Fe^3+ and SCN^-? b) What is the equilibrium constant for the reaction?
1. A student mixes 5.00 mL of 2.00 x 10 M Fe(NO3)3 with 5.0 mL of...
1. A student mixes 5.00 mL of 2.00 x 10 M Fe(NO3)3 with 5.0 mL of 2.00 x 10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.2 x 104 M. Find the Kc for the reaction of Fe (aq) + SCN (aq) → FeSCN2(aq) using the following steps. a. Find the initial concentration of Fe and SCN. (Use Equation 4). Record the value in the ICE Chart below. b. What is the equilibrium...
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by...
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by mixing these things in a 25.00 mL volumetric flask and then diluting to the volume of the flask with 0.3 M HNO3. 5.00 mL 0.00200 M NaSCN 10.00 mL 0.30 M Fe(NO3)3 What is the concentration of FeSCN2+ in this mixture? [Pay attention to the values to determine which reactant is being driven to completely react...] 2. You prepare a mixture to use to...
Fe3(aq) FESCN (aq) SCN (aq) In this experiment, we'll be examining the temperature-dependence of the rate constant...
Fe3(aq) FESCN (aq) SCN (aq) In this experiment, we'll be examining the temperature-dependence of the rate constant for the reaction above. 1. Using the UV-Vis instrument, you measured a room temperature absorbance for FESCN2 at 477 nm of 0.815. What is its concentration in molarity (M)? Please show all work. The molar absorptivity for FeSCN2 is 4,258 м"сm1 a. Answer: b. You calculated the [FeSCN2] above from the observed room temperature absorbance. Which one of the following statements about the...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C.
A student mixes 5.12 mL of 4.02 x 10...
Section Name Experiment 23 Advance Study Assignment: Determination of the Equilibrium Constant for a Chemical Reaction 1. A student mixes 5.00 mL 2.00 X 10M Fe(NO), with 5.00 ml 2.00 x 10-M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN is 1.40 x 10M. Find K for the reaction Fe(aq) + SCN (aq) FeSCN2(aq). Step 1 Find the number of moles Fe and SCN initially present. (Use Eq. 3.) (5.00 x103 LX (300X163) = (x 103...
A student mixes 5.00 mL of 2.00 times 10^-3 M Fe(NO_3)_3 with 5.00 mL of 2.00 times 10^-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2^+ is 1.40 times 10^-4 M. a) What is the initial concentration in solution of the Fe^3+ and SCN^-? b) What is the equilibrium constant for the reaction?
1. A student mixes 5.00 mL of 2.00 x 10 M Fe(NO3)3 with 5.0 mL of 2.00 x 10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.2 x 104 M. Find the Kc for the reaction of Fe (aq) + SCN (aq) → FeSCN2(aq) using the following steps. a. Find the initial concentration of Fe and SCN. (Use Equation 4). Record the value in the ICE Chart below. b. What is the equilibrium...
Fe3(aq) FESCN (aq) SCN (aq) In this experiment, we'll be examining the temperature-dependence of the rate constant for the reaction above. 1. Using the UV-Vis instrument, you measured a room temperature absorbance for FESCN2 at 477 nm of 0.815. What is its concentration in molarity (M)? Please show all work. The molar absorptivity for FeSCN2 is 4,258 м"сm1 a. Answer: b. You calculated the [FeSCN2] above from the observed room temperature absorbance. Which one of the following statements about the...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
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